The following reaction was carried out in a 2.50 L reaction vessel at 1100 K: C(
ID: 1040357 • Letter: T
Question
The following reaction was carried out in a 2.50 L reaction vessel at 1100 K:
C(s)+H2O(g)?CO(g)+H2(g)
B) If during the course of the reaction, the vessel is found to contain 5.75 mol of C, 16.0 mol of H2O, 4.00 mol of CO, and 7.50 mol of H2, what is the reaction quotient Q?
C) The reaction 2CH4(g)?C2H2(g)+3H2(g) has an equilibrium constant of K = 0.154.
If 6.60 mol of CH4, 4.80 mol of C2H2, and 10.75 mol of H2 are added to a reaction vessel with a volume of 5.20 L , what net reaction will occur?
Explanation / Answer
C(s) + H2O(g) ------------ CO(g) + H2(g)
volume = 2.50L
number of moles of C = 5.75 moles
number moles of H2O= 16.0 moles
number of moles of CO= 4.00 moles
number of moles of H2= 7.50 moles
concentration of C= number o fmoles/volume = 5.75/2.5 = 2.3M
concentration of H2O= 16.0/2.50=6.4M
concentration of CO= 4.00/2.50=1.6M
concentration of H2= 7.50/2.50 = 3.0M
Q= [CO][H2]/[C][H2O] = 1.6x3.0/2.3x6.4
Q= 0.326.
C)
2 CH4(g) ---------------- C2H2(g ) + 3 H2(g)
volume = 5.20L
Concentration of CH4= 6.60/5.20 = 1.269M
concentration of C2H2 = 4.80/5.20= 0.923M
Concentration of H2= 10.75/5.20 = 2.067
Q= [C2H2][H2]^3/[CH4]^2
Q= 0.923x(2.067)^3/(1.269^2
Q= 2.45
K= 0.154
Q > K
The reaction will proceed to the left.
i,e backword reaction can takesplace.
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